Chemical Equilibrium Pt. 4 Module Q. 14

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Lauren Huang 1H
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Joined: Fri Sep 28, 2018 12:16 am

Chemical Equilibrium Pt. 4 Module Q. 14

Postby Lauren Huang 1H » Mon Jan 14, 2019 12:12 am

14. The two air pollutants SO2 and NO2 can react in the atmosphere as follows:
SO2 (g) + NO2 (g) ⇌ SO3 (g) + NO (g)
Predict the effect of the following changes to the amount of NO when the reaction above has come to equilibrium in a stainless steel bulb equipped with entrants for chemicals.
i. The amount of NO2 is increased.
ii. The SO3 is removed by condensation.
iii. The pressure is tripled by pumping in helium.

Can someone please explain why removing SO3 causes the amount of NO to increase?

Katie_Duong_1D
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

Re: Chemical Equilibrium Pt. 4 Module Q. 14

Postby Katie_Duong_1D » Mon Jan 14, 2019 4:44 am

Le Chatelier's principle states that there is a tendency for systems in equilibrium to shift left or right to return back to its normal state. A decrease in SO3 would cause amounts of NO to increase because SO3 is a product like NO. If a product is decreased, then the forward reaction is preferred to shift the equation right. This produces more product, the amount of NO increases.


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